As we travel down a group, elements contain electrons further from their nuclei, and these electrons are bound less tightly. Electron proximity to these respective nuclei also influences this phenomenon, but contrary to the previous trend, electrons are placed in higher energy levels. Down GroupsĪs we travel down groups, electron affinities become more negative, meaning the process is more endothermic. These electrons exhibit a stronger attraction to the nuclei as a result of this proximity, explaining the exothermic nature of their electron affinities. Scientists attribute this pattern to the addition of electrons closer to the nuclei of these more rightward atoms.Īs elements trend to the right, the added electrons sit closer to their nuclei. Periodic Trends Across PeriodsĪs we travel from left to right on the periodic table, electron affinities become more positive- meaning that the electron attachment process is more exothermic. This results in positive second electron affinity values. This endothermic process requires more energy than is released when an electron is added to the system. The second pertains to the addition of an electron to a negative ion. Because this exothermic process releases energy, first electron affinities are negative values. The first involves the addition of an electron to a neutral atom. There are two types of electron affinity, first and second. Essentially, electron affinity pertains to the energy changes that accompany the gain of one electron, and ionization energy those that accompany losing one electron. Ionization energies always involve the formation of positive ions, electron affinity energies describe the generation of negative ions. It is the opposite of ionization energy, the energy required to ionize a gaseous atom and consequently remove an electron. We tend to liken electron affinity to an atom’s “likelihood,” or “chance,” of gaining an electron. This process differs from electronegativity, which we define as the ability of an atom to attract an electron toward itself. Topics Covered in Other ArticlesĬhemists define electron affinity as the change in energy, measured in units of kJ/mole, experienced when an electron is added to a gaseous atom. You can effortlessly find every single detail about the elements from this single Interactive Periodic table.In this tutorial about electron affinity, we will cover its definition, relevant periodic table trends, and factors that influence it. Let me tell you how this Interactive Periodic Table will help you in your studies.ġ). Free Gift for you: Interactive Periodic Table Note 2: If you want a periodic table with valence electrons labeled on it, then visit this article: Periodic table with Valence electrons (labeled on it)(From this article, you can also download the HD image of periodic table labeled with valence electrons, so visit right now). Note 1: If you want the valence electrons of all the 118 elements, then visit this article: Valence electrons chart for ALL ELEMENTS(Where I have shown the valence electrons using images). Atomic Number Element Valence electrons 1 Hydrogen (H) 1 2 Helium (He) 2 3 Lithium (Li) 1 4 Beryllium (Be) 2 5 Boron (B) 3 6 Carbon (C) 4 7 Nitrogen (N) 5 8 Oxygen (O) 6 9 Fluorine (F) 7 10 Neon (Ne) 8 11 Sodium (Na) 1 12 Magnesium (Mg) 2 13 Aluminum (Al) 3 14 Silicon (Si) 4 15 Phosphorus (P) 5 16 Sulfur (S) 6 17 Chlorine (Cl) 7 18 Argon (Ar) 8 19 Potassium (K) 1 20 Calcium (Ca) 2 21 Scandium (Sc) 2 22 Titanium (Ti) 2 23 Vanadium (V) 2 24 Chromium (Cr) 1 25 Manganese (Mn) 2 26 Iron (Fe) 2 27 Cobalt (Co) 2 28 Nickel (Ni) 2 29 Copper (Cu) 1 30 Zinc (Zn) 2 Valence electrons of first 30 elements of the Periodic table are mentioned below.
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